Explosive complexes

ABSTRACT

Lead-free primary explosives of the formula [M II (A) R (B X ) X ](C Y ) T , where A is 1,5-diaminotetrazole, and syntheses thereof are described. Substantially stoichiometric equivalents of the reactants lead to high yields of pure compositions thereby avoiding dangerous purification steps.

CROSS REFERENCE TO RELATED APPLICATION

The following is a divisional application of U.S. patent application Ser. No. 11/707,610, filed Feb. 15, 2007.

STATEMENT OF FEDERAL RIGHTS

The United States government has rights in this invention pursuant to Contract No. DE-AC51-06NA25396 between the United States Department of Energy and Los Alamos National Security, LLC for the operation of Los Alamos National Laboratory.

FIELD OF INVENTION

The present invention relates to lead-free primary explosives.

BACKGROUND

Explosives are categorized as primary or secondary based on their susceptibility to initiation. Primary explosives are highly susceptible to initiation and are used in small quantities to ignite secondary explosives, main charges, propellants, or fuel. Requirements for primary explosives include sufficient sensitivity to be detonated reliably while not being exceedingly dangerous to handle as well as sufficient thermal stability to not decompose on extended storage or thermal insult.

Two common primary explosives are lead azide and lead styphnate, but both emit toxic lead upon detonation. Because of this toxic residue, the development of a lead-free primary explosive is needed.

SUMMARY OF INVENTION

The present invention discloses novel lead-free compounds and syntheses thereof. More particularly, the present invention is directed to compounds of the formula [M^(II)(A)_(R)(B^(X))_(s)](C^(Y))_(T) and syntheses thereof, wherein

M is selected from the group consisting of

-   -   (1) cobalt,     -   (2) copper,     -   (3) iron,     -   (4) manganese,     -   (5) nickel, and     -   (6) zinc:

A is 1,5-diaminotetrazole (“DAT”);

B is selected from the group consisting of

-   -   (1) water (“H₂O”)     -   (2) 5-aminotetrazole (“AT”),     -   (3) 5-aminotetrazolate (“AT⁻”),     -   (4) 5-nitrotetrazolate (“NT⁻”),     -   (5) 3,5-dinitro-1,2,4-triazolate (“DNT⁻”),     -   (6) 5-azido-3-nitro-1,2,4-triazolate (“ANT⁻”),     -   (7) azide (“N₃ ⁻”), and     -   (8) nitrate (“NO₃ ⁻”);

C is selected from the group consisting of

-   -   (1) AT⁻,     -   (2) ANT⁻,     -   (3) DNT⁻,     -   (4) NO₃ ⁻,     -   (5) N₃ ⁻,     -   (6) NT⁻,     -   (7) perchlorate (“ClO₄ ⁻”),     -   (8) tetraazidoborate (“TAB⁻”),     -   (9) dinitramide (“DN⁻”),     -   (10) nitroformate (“NF⁻”),     -   (11) 5,5′-diazido-2,2′-azo-1,3,4-triazolate (“DAAT²⁻”),     -   (12) 5,5′-dinitro-2,2′-azo-1,3,4-triazolate (“DNAT²⁻”),     -   (13) 4,4′,5,5′-tetranitro-2,2′-biimidazolate (“TNBl²⁻”), and     -   (14) 5,5′-azotetrazolate (“AZT²⁻”),

R is 5 or 6;

S is 0 or 1;

T is 1 or 2;

X is 0 or −1;

Y is −1 or −2;

X+Y=−2; and

R+S=6.

The above compound can be prepared according to the reaction [M^(II)(H₂O)₆]D₂+R(A)+S(B^(X))+T(C^(Y))→[M^(II)(A)_(R)(B^(X))_(S)](C^(Y))_(T) wherein

M is selected from the group consisting of

-   -   (1) cobalt,     -   (2) copper,     -   (3) iron,     -   (4) manganese,     -   (5) nickel, and     -   (6) zinc;

A is DAT;

B is selected from the group consisting of

-   -   (1) H₂O,     -   (2) AT,     -   (3) AT⁻,     -   (4) NT⁻,     -   (5) DNT⁻,     -   (6) ANT⁻,     -   (7) N₃ ⁻, and     -   (8) NO₃ ⁻;

C is selected from the group consisting of

-   -   (1) AT⁻,     -   (2) ANT⁻,     -   (3) DNT⁻,     -   (4) NO₃ ⁻,     -   (5) N₃ ⁻,     -   (6) NT⁻,     -   (7) ClO₄ ⁻,     -   (8) TAB⁻,     -   (9) DN⁻,     -   (10) NF⁻,     -   (11) DAAT²⁻,     -   (12) DNAT²⁻,     -   (13) TNBI²⁻, and     -   (14) AZT²⁻;

D is selected from the group consisting of

-   -   (1) ClO₄ ⁻,     -   (2) NO₃ ⁻, and     -   (3) Cl⁻;

R is 5 or 6;

S is 0 or 1;

T is 1 or 2;

X is 0 or −1;

Y is −1 or −2;

X+Y=−2; and

R+S=6

as follows:

-   -   (1) mixing a chosen quantity of a metal salt [M^(II)(H₂O)₆]D₂         and R molar equivalents of A in a suitable solvent, thereby         forming a first solution;     -   (2) heating said first solution at a time and temperature         suitable for the color of said first solution to change;     -   (3) adding S molar equivalents of B^(X) to said first solution,         thereby forming a second solution;     -   (4) heating said second solution at a time and temperature         suitable for generating a third solution containing a cationic         complex;     -   (5) adding T molar equivalents of C^(Y) to said third solution         containing said cationic complex at a time and temperature         suitable to form said compound;     -   (6) cooling said third solution to room temperature; and     -   (7) separating said compound from said third solution.

BRIEF DESCRIPTION OF THE DRAWINGS

FIG. 1: (A) shows a copper embodiment of the lead-free compound [Cu^(II)(DAT)₅(H₂O)](ClO₄)₂. (B) shows a copper embodiment of the lead-free compound [Cu^(II)(DAT)₅(NO₃)]NO₃. (C) shows an iron embodiment of the lead-free compound [Fe^(II)(DAT)₆](ClO₄)₂. (D) shows a copper embodiment of the lead-free compound [Cu^(II)(DAT)₆](ClO₄)₂.

FIG. 2: (A) and (B) show two scanning electron microscope outputs for the copper embodiment of the lead-free compound [Cu^(II)(DAT)₅(H₂O)](ClO₄)₂. (A) has a magnification of 1,000. (B) has a magnification of 10,000. (C) and (D) show two scanning electron microscope outputs for the iron embodiment of the lead-free compound [Fe^(II)(DAT)₆](ClO₄)₂. (C) has a magnification of 1,000. (D) has a magnification of 10,000. (E) and (F) show two scanning electron microscope outputs for the copper embodiment of the lead-free compound [Cu^(II)(DAT)₆](ClO₄)₂. (E) has a magnification of 1,000. (F) has a magnification of 10,000.

DETAILED DESCRIPTION OF THE INVENTION

The present invention is directed to compounds of the formula [M^(II)(A)_(R)(B^(X))_(S)](C^(Y))_(T) and syntheses thereof, wherein

M is selected from the group consisting of

-   -   (1) cobalt,     -   (2) copper,     -   (3) iron,     -   (4) manganese,     -   (5) nickel, and     -   (6) zinc;

A is DAT;

B is selected from the group consisting of

-   -   (1) H₂O,     -   (2) AT,     -   (3) AT⁻,     -   (4) NT⁻,     -   (5) DNT⁻,     -   (6) ANT⁻,     -   (7) N₃ ⁻, and     -   (8) NO₃ ⁻;

C is selected from the group consisting of

-   -   (1) AT⁻,     -   (2) ANT⁻,     -   (3) DNT⁻,     -   (4) NO₃ ⁻,     -   (5) N₃ ⁻,     -   (6) NT⁻,     -   (7) ClO₄ ⁻,     -   (8) TAB⁻,     -   (9) DN⁻,     -   (10) NF⁻,     -   (11) DAAT²⁻,     -   (12) DNAT²⁻,     -   (13) TNBI²⁻, and     -   (14) AZT²⁻;

R is 5 or 6;

S is 0 or 1;

T is 1 or 2;

X is 0 or −1;

Y is −1 or −2;

X+Y=−2; and

R+S=6.

The above compound can be prepared according to the reaction [M^(II)(H₂O)₆]D₂+R(A)+S(B^(X))+T(C^(Y))→[M^(II)(A)_(R)(B^(X))_(S)](C^(Y))_(T) wherein

M is selected from the group consisting of

-   -   (1) cobalt,     -   (2) copper,     -   (3) iron,     -   (4) manganese,     -   (5) nickel, and     -   (6) zinc;

A is DAT;

B is selected from the group consisting of

-   -   (1) H₂O,     -   (2) AT,     -   (3) AT⁻,     -   (4) NT⁻,     -   (5) DNT⁻,     -   (6) ANT⁻,     -   (7) N₃ ⁻, and     -   (8) NO₃ ⁻;

C is selected from the group consisting of

-   -   (1) AT⁻,     -   (2) ANT⁻,     -   (3) DNT⁻,     -   (4) NO₃ ⁻,     -   (5) N₃ ⁻,     -   (6) NT⁻,     -   (7) ClO₄ ⁻,     -   (8) TAB⁻,     -   (9) DN⁻,     -   (10) NF⁻,     -   (11) DAAT²⁻,     -   (12) DNAT²⁻,     -   (13) TNBI²⁻, and     -   (14) AZT²⁻;

D is selected from the group consisting of

-   -   (1) ClO₄ ⁻,     -   (2) NO₃ ⁻, and     -   (3) Cl⁻,

R is 5 or 6:

S is 0 or 1;

T is 1 or 2;

X is 0 or −1;

Y is −1 or −2;

X+Y=−2; and

R+S=6

as follows:

-   -   (1) mixing a chosen quantity of a metal salt [M^(II)(H₂O)₆]D₂         and R molar equivalents of A in a suitable solvent, thereby         forming a first solution:     -   (2) heating said first solution at a time and temperature         suitable for the color of said first solution to change;     -   (3) adding S molar equivalents of B^(X) to said first solution,         thereby forming a second solution;     -   (4) heating said second solution at a time and temperature         suitable for generating a third solution containing a cationic         complex;     -   (5) adding T molar equivalents of C^(Y) to said third solution         containing said cationic complex at a time and temperature         suitable to form said compound;     -   (6) cooling said third solution to room temperature; and     -   (7) separating said compound from said third solution.

In step 1, a suitable solvent is an ethanolic solvent or an acidic ethanolic solvent (a mixture of absolute ethanol and two drops of acid with a pH measurement ranging from about 0 to about 2). In step 4, the second solution can be heated anywhere from about above room temperature to reflux and for a time in the range of from about 30 minutes to 3 hours or until the solution becomes colorless. In step 6, the third solution is preferably slowly cooled to 40° C. with gentle stirring, and then the third solution is allowed to cool to room temperature undisturbed. Gentle stirring can achieve small particle sizes for subsequent safe handling. Depending on the nature of C^(Y), the ethanolic reaction solution may be reduced in volume, or the temperature is lowered using an ice-bath to precipitate the compound.

Dangerous purification steps can be avoided by employing an absolute ethanolic solvent and stoichiometric equivalents of the reactants to form a nearly quantitative single product. An acidic solvent or excess quantity of any reactant might result in impurities.

Reference is now made in detail to four embodiments of the invention. These four embodiments are [Cu^(II)(DAT)₅(H₂O)](ClO₄)₂, [Cu^(II)(DAT)₅(NO₃)]NO₃, [Fe^(II)(DAT)₆](ClO₄)₂, and [Cu^(II)(DAT)₆](ClO₄)₂ which may have the configurations shown in FIGS. 1A-1D.

The embodiment of [Cu^(II)(DAT)₅(H₂O)](ClO₄)₂ can be prepared by refluxing a solution of copper salt having the formula [Cu^(II)(H₂O)₆](ClO₄)₂ and 5 molar equivalents of DAT in a suitable solvent. The resulting precipitate is filtered and washed thoroughly with fresh, cold ethanol. The reaction gives nearly quantitative yield and an analytically pure product of [Cu^(II)(DAT)₅(H₂O)](ClO₄)₂ without additional recrystallization or purification.

The embodiment of [Cu^(II)(DAT)₅(NO₃)]NO₃ can be prepared by refluxing a solution of a copper salt having the formula [Cu^(II)(H₂O)₆](NO₃)₂ and 5 molar equivalents of DAT in a suitable solvent. The resulting precipitate is filtered and washed thoroughly with fresh, cold ethanol. The reaction gives nearly quantitative yield and an analytically pure product of [Cu^(II)(DAT)₅(NO₃)]NO₃ without additional recrystallization or purification.

The embodiment of [Fe^(II)(DAT)₆](ClO₄)₂ can be prepared by refluxing a solution of an iron salt having the formula [Fe^(II)(H₂O)₆](ClO₄)₂ and 6 molar equivalents of DAT in a suitable solvent. The resulting precipitate is filtered and washed thoroughly with fresh, cold ethanol. The reaction gives nearly quantitative yield and an analytically pure product of [Fe^(II)(DAT)₆](ClO₄)₂ without additional recrystallization or purification.

The embodiment of [Cu^(II)(DAT)₆](ClO₄)₂ can be prepared by refluxing a solution of a copper salt having the formula [Cu^(II)(H₂O)₆](ClO₄)₂ and 6 molar equivalents of DAT in a suitable solvent. The resulting precipitate is filtered and washed thoroughly with fresh, cold ethanol. The reaction gives nearly quantitative yield and an analytically pure product of [Cu^(II)(DAT)₆](ClO₄)₂ without additional recrystallization or purification.

Example 1 Preparation of [Cu^(II)(DAT)₅(H₂O)](ClO₄)₂

A copper compound was prepared in accordance with the reaction [Cu^(II)(H₂O)₆](ClO₄)₂+5DAT→[Cu^(II)(DAT)₅(H₂O)](ClO₄)₂ as follows:

-   -   (a) 0.15 grams (“g”) of cupric perchlorate was completely         dissolved in 40 milliliters (“mL”) of absolute ethanol;     -   (b) 0.203 g of DAT was slowly added to the solution of cupric         perchlorate;     -   (c) the resulting solution was heated to reflux for between 2         hours and 3 hours or until the mother liquor was completely         clear and colorless;     -   (d) the solution was cooled to about 40° C. with slow stirring         and then allowed to cool to room temperature undisturbed;     -   (e) the precipitate was filtered out of the mother liquor,         thereby accumulating a collected solid;     -   (f) the collected solid was washed thoroughly with fresh, cold,         absolute ethanol;     -   (g) the undried collected solid was wet transferred into a         Teflon-vial using a plastic spatula with care taken to avoid         scraping or friction between the spatula and walls of the vial;         and     -   (h) the collected solid was air-dried prior to use.

Elemental analysis of the collected solid, as set forth in TABLE 1 showed the composition corresponds to [Cu^(II)(DAT)₅(H₂O)]ClO₄)₂.

TABLE 1 CARBON (%) HYDROGEN (%) NITROGEN (%) THEORETICAL 7.69 2.84 53.81 OBSERVED 7.54 ± 0.4 2.57 ± 0.4 51.18 ± 0.4

The above-described synthesis yielded about 91% [Cu^(II)(DAT)₅(H₂O)](ClO₄)₂.

FIG. 2A shows two scanning electron microscope outputs for the copper embodiment of the lead-free compound [Cu^(II)(DAT)₅(H₂O)](ClO₄)₂.

The left output has a magnification of 1,000. The right output has a magnification of 10,000.

The density of the copper compound was 1.98 grams per cubic centimeter (“g/cm³”) using a liquid pycnometry technique. The thermal decomposition temperature was 224° C. (on a 5-7 microgram (“μg”) sample) as determined by Differential Scanning calorimetry (“DSC).

Explosive initiation data of the dry collected solid were as follows:

-   Friction: 15 g determined on a 1-1.5 milligram (g”) sample using     mini BAM: -   Impact: 5 cm on a 5 mg sample determined by a type 12 impact     machine; -   Spark: 0.06875 joules (“J”) determined by ABL Electrostatic     Discharge.

Example 2 Preparation of [Cu^(II)(DAT)₅(NO₃)]NO₃

A copper compound was prepared in accordance with the reaction [Cu^(II)(H₂O)₆](NO₃)₂+5DAT→[Cu^(II)(DAT)₅(NO₃)]NO₃ as follows:

-   -   (a) 0.30 g of cupric nitrate was completely dissolved in 40 mL         of absolute ethanol;     -   (b) 0.405 g of DAT was slowly added to the solution of cupric         nitrate;     -   (c) the resulting solution was heated to reflux for between 2         hours and 3 hours or until the mother liquor was completely         clear and colorless;     -   (d) the solution was cooled to about 40° C. with slow stirring         and then allowed to cool to room temperature undisturbed;     -   (e) the precipitate was filtered out of the mother liquor,         thereby accumulating a collected solid;     -   (f) the collected solid was washed thoroughly with fresh, cold,         absolute ethanol;     -   (g) the undried collected solid was wet transferred into a         Teflon-vial using a plastic spatula with care taken to avoid         scraping or friction between the spatula and walls of the vial;         and     -   (h) the collected solid was air-dried prior to use.

Elemental analysis of the collected solid, as set forth in TABLE 2, showed the composition corresponds to [Cu^(II)(DAT)₅(NO₃)]NO₃.

TABLE 2 CARBON (%) HYDROGEN (%) NITROGEN (%) THEORETICAL 8.73 2.93 65.15 OBSERVED 8.77 ± 0.4 2.82 ± 0.4 63.23 ± 0.4

The above-described synthesis yielded about 94% [Cu^(II)(DAT)₅(NO₃)]NO₃.

The density of the copper compound was 2.08 g/cm³ using a liquid pycnometry technique. The thermal decomposition temperature was 228° C. (on a 7-8 μg sample) as determined by DSC.

Explosive initiation data of the dry collected solid were as follows:

Friction: 2.0 kg determined on a 1-1.5 mg sample using BAM; Impact: 10 cm on a 5 mg sample determined by a type 12 impact machine; Spark: 3.125 J determined by ABL Electrostatic Discharge.

Example 3 Preparation of [Fe^(II)(DAT)₆](ClO₄)₂

An iron compound was prepared in accordance with the reaction [Fe^(II)(H₂O)₆](ClO₄)₂+6DAT→[Fe^(II)(DAT)₆](ClO₄)₂ as follows:

-   -   (a) 0.20 g of ferrous perchlorate was completely dissolved in 40         mL of absolute ethanol:     -   (b) 0.331 g of DAT was slowly added to the solution of ferrous         perchlorate;     -   (c) the resulting solution was heated to reflux for between 2         hours and 3 hours or until the mother liquor was completely         clear and colorless;     -   (d) the solution was cooled to about 40° C. with slow stirring         and then allowed to cool to room temperature undisturbed;     -   (e) the precipitate was filtered out of the mother liquor,         thereby accumulating a collected solid;     -   (f) the collected solid was washed thoroughly with fresh, cold,         absolute ethanol;     -   (g) the undried collected solid was wet transferred into a         Teflon-vial using a plastic spatula with care taken to avoid         scraping or friction between the spatula and walls of the vial;         and     -   (h) the collected solid was air-dried prior to use.

Elemental analysis of the collected solid, as set forth in TABLE 3, showed the composition corresponds to [Fe^(II)(DAT)₆](ClO₄)₂.

TABLE 3 CARBON (%) HYDROGEN (%) NITROGEN (%) THEORETICAL 8.43 2.83 58.96 OBSERVED 8.60 ± 0.4 2.92 ± 0.4 58.23 ± 0.4

The above-described synthesis yielded about 93% [Fe^(II)(DAT)₆](ClO₄)₂.

FIG. 2B shows two scanning electron microscope outputs for the iron embodiment of the lead-free compound having a formula [Fe^(II)(DAT)₆](ClO₄)₂. The left output has a magnification of 1,000. The right output has a magnification of 10,000.

The density of the iron compound was 2.03 g/cm³ using a liquid pycnometry technique. The thermal decomposition temperature was 194° C. (on a 4-5 μg sample) as determined by DSC.

Explosive initiation data of the dry collected solid were as follows:

Friction: <10 g determined on a 1-1.5 mg sample using mini BAM; Impact: 5 cm on a 5 mg sample determined by a type 12 impact machine; Spark: 0.0375 J determined by ABL Electrostatic Discharge.

Example 4 Preparation of [Cu^(II)(DAT)₆](ClO₄)₂

A copper compound was prepared in accordance with the reaction [Cu^(II)(H₂O)₆](ClO₄)₂+6 DAT→[Cu^(II)(DAT)₆](ClO₄)₂ in a manner similar to that described in EXAMPLE 1 for the preparation of [Cu^(II)(DAT)₅(H₂O)](ClO₄)₂ herein above, except that 6 molar equivalents of DAT are used in step (b).

Elemental analysis of the collected solid, as set forth in TABLE 4, showed the composition corresponds to [Cu^(II)(DAT)₆](ClO₄)₂.

TABLE 4 CARBON (%) HYDROGEN (%) NITROGEN (%) THEORETICAL 8.35 2.80 58.43 OBSERVED 7.97 ± 0.4 2.64 ± 0.4 54.43 ± 0.4

The above-described synthesis yielded about 94% [Cu^(II)(DAT)₆](ClO₄)₂.

FIG. 2C shows two scanning electron microscope outputs for a copper embodiment of the lead-free compound having a formula [Cu^(II)(DAT)₆](ClO₄)₂. The left output has a magnification of 1,000. The right output has a magnification of 10,000.

The density of the copper compound was 2.14 g/cm³ using a liquid pycnometry technique. The thermal decomposition temperature was 232° C. (on a 4-5 μg) as determined by DSC.

Explosive initiation data of the dry collected solid were as follows:

Friction: <10 g determined on a 1-1.5 mg sample using mini BAM; Impact: 5 cm on a 5 mg sample determined by a type 12 impact machine; Spark: 0.03125 J determined by ABL Electrostatic Discharge.

It is understood that the foregoing detailed description and examples are merely illustrative and are not to be taken as limitations upon the scope of the invention, which is defined by the appended claims. Various changes and modifications to the disclosed embodiments will be apparent to those skilled in the art. Such changes and modifications, including without limitation those relating to chemical structures, syntheses, formulations and/or methods of use of the invention, may be made without departing from the spirit and scope thereof. 

1. A process for preparing a compound according to the reaction [M^(II)(H₂O)₆]D₂+R(A)→[M^(II)(A)_(R)(H₂O)_(6-R)(D)_(X)](D)_(2-X) M is selected from the group consisting of (1) cobalt, (2) copper, (3) iron, (4) manganese, (5) nickel, and (6) zinc; A is DAT; D is selected from the group consisting of (1) ClO₄ ⁻, (2) NO₃ ⁻, and (3) Cl⁻; R is 5 or 6; and X is 0 or 1; and R+X=6 as follows: (1) mixing a chosen quantity of a metal salt [M^(II)(H₂O)₆]D₂ and R molar equivalents of A in a suitable solvent, thereby forming a solution; (2) heating said solution at a time and temperature suitable for the color of said solution to change; (3) cooling said solution to room temperature to form a precipitate of the compound; and (4) filtering the precipitate of the compound.
 2. The process of claim 1 wherein R is
 6. 3. The process of claim 1 wherein M is iron.
 4. The process of claim 1 wherein R is
 5. 5. (canceled)
 6. The process of claim 1 wherein said suitable solvent is an ethanolic solvent.
 7. The process of claim 1 wherein said second solution is heated in p step 2 to reflux for between 2 to 3 hours or until clear and colorless.
 8. The process of claim 1 wherein said solution is cooled in step 2 to around 40° C. with gentle stirring and then cooled to room temperature undisturbed. 